Using the following data, determine the standard cell potential e^o cell for the electrochemical cell constructed using the following reaction, where zinc is the anode and lead is the cathode.

zn(s) + pb2+(aq) -> zn2+(aq) + pb(s)

half-reaction: standard reduction potential:

zn2+(aq) + 2e- -> zn(s)= -0.763

pb2+(aq) + 2e- -> pb(s)= -0.126

a. -0.889 v

b. +0.889 v

c. +0.637 v

d. +1.274 v

e. -0.637 v

C)  0.637 V

Explanation:

The balanced redox reaction is:

Here Zn undergoes oxidation by loss of electrons, thus act as anode. Lead undergoes reduction by gain of electrons and thus act as cathode.

Where both are standard reduction potentials.

= -0.763

= -0.126

The standard emf of a cell is 0.637 V

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